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ATOMIC STRUCTURE
ATOMIC MASS UNIT(a.m.u.)
A system of mass measurement used for extremely tiny particles (such as the parts of an atom)1 a.m.u. = 1.66 x 10-24g = .00000000000000000000000166 gWhich would you rather write?
The positively charged “center” of an atom
Virtually ALL of an atom’s mass is located in the nucleus
Composed of protons and neutrons
NUCLEUS
PROTONS
Positively charged particles that are located in the nuclei of atoms
Mass = 1 atomic mass unit (a.m.u.)
NEUTRONS
Uncharged particles located in the nuclei of atoms
Mass = 1 a.m.u.
ELECTRONS
Negatively charged particles that surround (orbit) the nuclei of atoms
Electrons have virtually NO mass: Mass = 0 a.m.u.
Let’s Synthesize!
Bohr Model of Oxygen
Number of Protons
Number of Neutrons
Nucleus
Electron
Energy Levels
Smaller particles of matter....Quarks
Scientists hypothesize that electrons are not make up of even smaller particles, however, protons and neutrons are!
The particles are called quarks.
At the present time, scientists believe that three quarks make up a proton, and three quarks make up a neutron.
The Tevatron is the most powerful proton-antiproton accelerator in the world. It accelerates beams of protons and antiprotons to 99.99999954 percent of the speed of light around a four-mile circumference. The two beams collide at the centers of two 5,000-ton detectors positioned around the beam pipe at two different locations. The collisions reproduce conditions in the early universe and probe the structure of matter at a very small scale.
The Tevatron
Finding the sixth quark took a team of nearly 450 scientists several years.
The collisions of protons with oppositely charged particles at high energies were necessary to produce the sixth quark.
This sixth quark is typically referred to as the "Top Quark".
ISOTOPE
Atoms of the same element that have different numbers of neutrons
NeutronsNeutronsNucleusNucleus ElectronsElectronsProtonsProtons
Label the diagram of the atomLabel the diagram of the atom
Click herefor theanswer
Click herefor theanswer
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Protons
ElectronsNucleus
Neutrons
The structure of an atom
Click hereto go back
Click hereto go back
Protons
ElectronsNucleus
Neutrons
The structure of an atom
Atomic Number equal the number of protons and determines the element’s place in the Periodic Table.
Atomic Weight equals the weight of an atom compared with the weight of an atom of carbon 12.
Atomic Mass or Mass Number equals the number of neutrons and protons. This number is very close to the atomic weight.
Electrons are orbiting the nucleus in a specific order.
Periods and Groups on the P. T.
Read the handout "Supersize the Atom".
Complete Periodic Table Practice sheet for homework.
Finish the Element Challenge Sheet!
Element Symbol
Atomic #
AtomicMass
Metal, nonmetal, metalloid
Characteristic and uses
1. Hydrogen
H 1 1.008 non metal most abundant element in Uwelding, fuel cell
2. Carbon
C 6 12.011 non metal diamonds,graphite, LIFE!
3. Oxygen
O 8 15.999 non metal
4. Silicon
Si 14 28.086 non metal
5. Iron Fe 26 55.845 metal
6. Krypton
Kr 36 83.80 non metal
7. Chlorine
Cl 17 35.453 non metal
8. Plutonium
Pu 94 (244) metal
9. Lead Pb 82 207.2 metal
10. Silver
Ag 47 107.363 metal
Protons, Neutrons and Electrons
Protons and neutrons are located inside the nucleus. Electrons are located in shells or energy levels
and orbit or move around the nucleus.
Energy Level
Shell Letter
Electron Capacity
1 K 2
2 L 8
3 M 18
4 N 32
5 O 50
6 P 72
3 Rules to Remember!
1. # of Protons = # of Electrons P=E
2. Atomic number equals number of protons
3. Atomic mass or mass number equals number of protons and number of neutrons
Name________________
Symbol_______________
Atom Number_________
Atom Mass___________
#of Protons___________
# of Electrons_________
# of Neutrons_________
Electron Configurations
Name________________
Symbol_______________
Atom Number_________
Atom Mass___________
#of Protons___________
# of Electrons_________
# of Neutrons_________
Name________________
Symbol_______________
Atom Number_________
Atom Mass___________
#of Protons___________
# of Electrons_________
# of Neutrons_________
Name________________
Symbol_______________
Atom Number_________
Atom Mass___________
#of Protons___________
# of Electrons_________
# of Neutrons_________
Name________________
Symbol_______________
Atom Number_________
Atom Mass___________
#of Protons___________
# of Electrons_________
# of Neutrons_________
Name________________
Symbol_______________
Atom Number_________
Atom Mass___________
#of Protons___________
# of Electrons_________
# of Neutrons_________
Name________________
Symbol_______________
Atom Number_________
Atom Mass___________
#of Protons___________
# of Electrons_________
# of Neutrons_________
Name________________
Symbol_______________
Atom Number_________
Atom Mass___________
#of Protons___________
# of Electrons_________
# of Neutrons_________
Name________________
Symbol_______________
Atom Number_________
Atom Mass___________
#of Protons___________
# of Electrons_________
# of Neutrons_________
Name________________
Symbol_______________
Atom Number_________
Atom Mass___________
#of Protons___________
# of Electrons_________
# of Neutrons_________
Name________________
Symbol_______________
Atom Number_________
Atom Mass___________
#of Protons___________
# of Electrons_________
# of Neutrons_________
Name________________
Symbol_______________
Atom Number_________
Atom Mass___________
#of Protons___________
# of Electrons_________
# of Neutrons_________
Pre 1980 pennies needed for Friday. Bring 2 pennies in.
Name________________
Symbol_______________
Atom Number_________
Atom Mass___________
#of Protons___________
# of Electrons_________
# of Neutrons_________
Ca
20
20
WITHOUT USING A PERIODIC TABLE, COMPLETE THE FOLLOWING AND DRAW THE ELECTRON CONFIGURATION.
GL
N
U
F
D
TM
A
Q
S
P
H
V
X
JC
BK
Y
R
IOWE
Solid sodium hydroxide or solutions of sodium hydroxide will cause chemical burns , permanent injury or scarring if it contacts unprotected human, or other animal, tissue. It will cause blindness if it contacts with the eye. Protective equipment such as eye protection should always be used when handling the material or its solutions.
Gold and Silver Pennies (or How to be an Alchemist) Lab
Safety: This lab requires safety goggles!! The strong heated base can severely damage your eyes and skin. Much caution is required during the entire lab!!
Gold and Silver Pennies (or How to be an Alchemist) Lab
Safety: This lab requires safety goggles!! The strong heated base can severely damage your eyes and skin. Much caution is required during the entire lab!!
Materials: Strong base solution (NaOH), zinc powder, alcohol burner and stand, 100 ml beaker, balance and weighing paper, graduated cylinder, forceps, beaker tongs, crucible tongs, two pennies dated earlier than 1980 per person (total 4 pennies)
Procedure for Part I:Measure 25 mL of base solution in a graduated cylinder and pour it into the beaker.Light the burner and set it under the stand.Put the beaker on the stand and start heating it.Measure 1.0 g of zinc powder on a balance, using the weighing paper technique. Pour the zinc powder into the strong base.Put one copper penny PER PERSON into the hot base solution.Stir the pennies for 3 minutes with forceps. WARNING: Do not let the solution boil. Don’t breathe the fumes. Be careful to not spill the base solution! Remove the pennies with a forceps and rinse in cold running water for a count of 20 seconds. Remove caked-on zinc with fingers. Set your “silver” pennies aside.
Procedure for Part II:1. Put one copper penny per person again into the hot base.2. Stir the pennies again for another 3 minutes.3. Take out the pennies and rinse in cold water again for 20 seconds.Dry the pennies, making sure the caked on zinc is gone. Use a crucible tong to hold one penny at a time in the flame of your burner. Do this until the penny turns “gold”. Don’t leave your pennies in the flame too long or they will not be shiny. Each person should now also have a “gold” penny.
Clean up: Wear your goggles. Pour the base solution down the sink with plenty of running water. Rinse your graduated cylinder. Wipe up your lab area.
Answer the questions on the back to complete this lab.
A homogeneous mixture or solid solution of two or more metals.
Alloy
Examples: magnelium - magnesium and aluminum used for making balances.
brass- copper and zinc
bronze- copper and tin
sterling silver- copper and silver
solder- tin and lead
Materials with a Past
1. What is an alloy?2. Why is an alloy a homogeneous
mixture?3. What is brass?
4. What is bronze?5. Name two more alloys containing
copper.6. What is an amalgam?
7. What do all steel alloys have in common?
Questions:
1. What are the modern abbreviations for the above elements? Zinc _________ Copper _______ Tin __________ Lead __________
2. How are elements different from mixtures? ___________________________________ ___________________________________________________________________________ 3. How many different elements does it take to make a mixture? _________________
4. Would this drawing represent an element or a mixture? _______________________
5. How many atoms are drawn above (see C.) for each mixture? Brass ____________ Bronze _____________ Solder ______________
6. How many different elements does it take to make each of the alloys drawn above? Brass __________ Bronze __________ Solder ___________
7. What element coats the “silver” penny you made in lab? ____________________
8. What alloy coats the “gold” penny? ____________________________
9. Draw an alloy of the elements zinc, copper, and tin made up of ten total atoms, using the Dalton Models above.
10. Sterling silver is an alloy of silver and copper. Make up a drawing of a sample of sterling silver, using 10 atoms. (You’ll have to think of a way to represent silver atoms first.)
Alloy Metals Uses
Brass Copper, zinc Hardware, musical instruments
Bronze Copper, tin Art, buildings
Pewter Tin, copper, bismuth, antimony
Art, dinnerware, candlesticks
Solder Lead, tin Connecting metal pieces together
Stainless steel Iron, chromium, nickel
Silverware, knives
An ALLOY is a mixture of metals. They are mixed when the metals are melted together, but there is NOT a chemical reaction between the atoms. Some common alloys are in the table below. Alloys have very different properties than the individual metals that make them up.
1. How many different elements does it take to make an alloy?
2. How many elements are in the alloys…
Brass? ___ Bronze? ___ Pewter?___ Stainless Steel? _____
3. Stainless steel is what your silverware and knives are made of. Why is the alloy stainless steel better for silverware than pure iron?
4. What ALLOY coats the “gold” penny you made in lab? Hint- you melted one metal into another metal. _____________________
5. A copper atom has ____ protons in its nucleus. It has _____ electrons outside its nucleus. It also has ____ neutrons in its nucleus. A copper atom’s atomic number is ______ and its mass number is _________.
ALCHEMY was practiced back in the Dark Ages, before there was “real” science. Alchemists had two goals: 1 - to discover a substance that could make them live forever, and 2 - to figure out how to turn cheap metals such as lead and zinc into valuable gold.
Imagine trying to turn lead into solid gold! They were never successful of course. But, they did learn very much about properties of metals and reactions, even if they didn’t really understand the science behind it.
